- "Chemical equilibrium is the state in which both the reactants and products are present in concentrations which have no further tendency to change with time."
The state in which the rates of the forward and reverse reactions are equal and the concentrations of the reactants and products remain constant.
Chemical Equations: Writing and Balancing: Chemical equations represent the reaction between reactants and products in a balanced manner.
Law of Mass Action: Law of Mass Action states that the rate of a chemical reaction is directly proportional to the concentration of reactants or products present.
Equilibrium Constant: The equilibrium constant is a ratio of the product concentration to the reactant concentration at equilibrium, with an additional factor of concentration equality in the reaction.
Le Chatelier's Principle: Le Chatelier's Principle explains the effect of concentration or pressure changes on the equilibrium state of a reaction.
Equilibrium Expressions: Equilibrium expressions represent the equilibrium constant in terms of the concentration of the species involved in the reaction.
Heterogeneous Equilibrium: Heterogeneous equilibrium is a state where the reactants and products are present in different phases, such as solid or liquid states.
Acid-Base Equilibria: Acid-Base Equilibria are chemical reactions where acids and bases react with each other resulting in the formation of water and salt in some cases.
Reaction Quotient: The reaction quotient is a ratio of the product of concentration of products to the concentration of reactants present in a chemical reaction at any instant except at equilibrium.
Ionization Constants: The ionization constants represent the equilibrium constant for ionization reactions.
Equilibrium Constant Expression for Gases: The equilibrium constant expression for gases is different from other reactions as it takes into account the partial pressure of each gas species.
Gibbs Energy Change and Chemical Equilibrium: Gibbs Energy Change is a thermodynamic property that explains the spontaneity or non-spontaneity of a chemical reaction.
Equilibrium Constant and Concentration: The concentration of the species involved in the reaction affects the equilibrium constant of the reaction.
Henry's Law: Henry's Law explains the relationship between the concentration of gas in a solution and its partial pressure.
Thermal Equilibria: Thermal Equilibria are chemical reactions where the energy exchange leads to temperature changes.
Kinetics of Chemical Equilibrium: Kinetics of Chemical Equilibrium explains the rate of reaction and how it influences the equilibrium point.
Equilibrium and Ionic Strength: The ionic strength of a solution plays a vital role in the equilibrium constant of an ionic reaction.
Factors Affecting Chemical Equilibrium: Factors such as temperature, pressure, and concentration affect the equilibrium state of a reaction.
Phase Equilibria: Phase Equilibria are a state where different phases coexist in a system but have the same physical and chemical properties in equilibrium.
Equilibrium and Solubility: The solubility of a compound affects the equilibrium constant of chemical reactions involving the compound.
Equilibrium and pH: The pH of a solution affects the equilibrium constant of acid-base reactions.
Homogeneous equilibrium: A homogeneous equilibrium occurs when all the reactants and products are in the same phase. For example, the reaction between hydrogen gas and iodine gas to form hydrogen iodide gas.
Heterogeneous equilibrium: A heterogeneous equilibrium occurs when the reactants and products are in different phases. For example, the combustion of coal to form carbon dioxide and water vapor.
Acid-base equilibrium: This equilibrium occurs when an acid and a base react to form water and a salt. For example, the reaction between hydrochloric acid and sodium hydroxide to form sodium chloride and water.
Oxidation-reduction equilibrium: An oxidation-reduction equilibrium occurs when electrons are transferred between reactants. For example, the reaction between copper and silver ions to form copper ions and silver.
Precipitation equilibrium: A precipitation equilibrium occurs when two soluble salts react to form an insoluble precipitate. For example, the reaction between silver nitrate and sodium chloride to form silver chloride, which is insoluble.
Complex ion equilibrium: A complex ion equilibrium occurs when an ion bonds to one or more ligands to form a complex ion. For example, the reaction between water and copper ions to form a blue-colored complex ion.
Gas equilibria: This equilibrium occurs when gas molecules interact with each other. For example, the reaction between carbon dioxide and water to form carbonic acid in a soda.
Solubility equilibrium: A solubility equilibrium occurs when a solid solute dissolves in a solvent. For example, the equilibrium between solid magnesium sulfate and water to form a solution of magnesium and sulfate ions.
Association-dissociation equilibrium: Association-dissociation equilibrium occurs when molecules come together or break apart. For example, the reaction between hydrogen ion and water molecules to form the hydronium ion and hydroxide.
Isomerization equilibrium: An isomerization equilibrium occurs when isomers are formed in reactions. For example, the reaction between ring-shaped molecules to form a new group of molecules.
Redox equilibrium: Redox equilibrium occurs when metals which displace each other interchange their electrons. For example, the electro-chemical reaction of Zinc and Copper.
Photochemical Equilibrium: This type of equilibrium proceeds in the presence of light. Common examples include the reactions during photosynthesis.
Ionic Equilibrium: Ionic Equilibrium refers to the balance of ions in a solution. This type of reaction is similar to Acid-Base equilibrium. Examples include reactions of Acidic and Basic Salts.
- "This state results when the forward reaction proceeds at the same rate as the reverse reaction."
- "The reaction rates of the forward and backward reactions are generally not zero."
- "They are equal."
- "There are no net changes in the concentrations of the reactants and products."
- "Such a state is known as dynamic equilibrium."
- "There is no observable change in the properties of the system."
- "Both the reactants and products are present in concentrations which have no further tendency to change with time."
- "The forward reaction proceeds at the same rate as the reverse reaction."
- "There are no net changes in the concentrations of the reactants and products."
- No direct quote in the paragraph, but can be inferred as a characteristic of chemical processes.
- "There is no observable change in the properties of the system."
- "Such a state is known as dynamic equilibrium."
- "Both the reactants and products are present in concentrations which have no further tendency to change with time."
- "The forward reaction proceeds at the same rate as the reverse reaction."
- "Both the reactants and products are present in concentrations which have no further tendency to change with time."
- "Both the reactants and products are present in concentrations which have no further tendency to change with time."
- No direct quote in the paragraph about the consequences, but it would indicate the system is not at equilibrium.
- "Both the reactants and products are present in concentrations which have no further tendency to change with time."
- "Both the reactants and products are present in concentrations which have no further tendency to change with time."